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The Atom

The Atom. How big are subatomic particles in relationship to one another and to the whole atom? Where are the subatomic particles located within the atom? What are the charges of the subatomic particles? Which atomic theory is most current?

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The Atom

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  1. The Atom

  2. How big are subatomic particles in relationship to one another and to the whole atom? Where are the subatomic particles located within the atom? What are the charges of the subatomic particles? Which atomic theory is most current? Which atomic theory states that electrons are in clouds? What is Dalton’s contribution to chemistry? Who discovered that electrons are negatively charged? What was the name of Rutherford’s experiment why was it so important? Whose model is like the planetary model? What are differences between Bohr’s model and the wave-mechanical model of the atom? What is the mass number equal to? What is the atomic number equal to? How do you write the symbols for isotopes of the same element? How do you calculate atomic mass? When is an atom neutral? Where are valence electrons found? What do the chemical properties of an element depend on? How are ions formed and how are they written? How do you write an equation that shows magnesium losing electrons? How do you write an equation that shows phosphorous gaining electrons? Why do ions form? Counting subatomic particles for neutral atoms and ions How do you draw a Lewis dot diagram for a neutral atom, a cation, and an anion? What is the relationship between an electron’s energy and its distance to the nucleus? What do electrons do when they gain energy? What do electrons do when they lose energy? How can you tell the difference between an atom in the excited state and an atom in the ground state? Recognize an emission spectrum and an absorption spectrum. Identify an element based on its spectrum. Concepts to Master

  3. Absorption spectrum Anion Atom Atomic mass Atomic number Cation Chemical property Compound Continuous spectrum Dual nature concept Electromagnetic spectrum Electron Electron configuration Emission spectrum Excited state Ground state Ionic charge Ions Isotope Mass number Matter Neutron Nucleus Octet rule Orbitals Orbits Oxidation number Proton Subatomic particle Valence electrons Valence shell Vocab

  4. Labs • Atomic Structure • Atomic Mass of Beadrock • Atomic Spectrum

  5. The Atom • The smallest component of an element. • So if there are103 different elements there are 103 different types of atoms. • Basic unit of all matter. • Matter is anything that has mass and volume.

  6. Subatomic Particles Nucleons located in the Nucleus of an atom • Protons • Neutrons • Electrons • Mass • electron mass = 9.10938188 × 10-31 kg • neutron mass = 1.6749286 × 10-27 kg • proton mass = 1.67262158 × 10-27 kg • amu • Atomic mass unit • 1 amu = mass of 1 proton • 1 amu = mass of 1 neutron • Easier for scientists to write in terms of amu • Mass of an electron is approximately 1/1836 of the mass of a proton or 1/1836 th of an amu.

  7. Proton - skyscraper Electron - Rat at the bottom of the skyscraper

  8. Atomic Structure Theories • Dalton • atoms are the basic units of matter • JJ Thompson • Plum pudding where the raisin are electrons • Rutherford • Atoms are mostly empty space • Bohr • Electrons are located in specific orbits around the nucleus • Wave Mechanical Model • Electrons exist in “clouds” around the nucleus Pg 66-69

  9. Dalton • Elements are composed of extremely small particles called atoms. • All atoms of a given element have identical properties. • Compounds are formed when atoms of different elements combine with one another in small whole numbers. • The relative numbers and kinds of atoms are constant in a given compound.

  10. Dalton’s Elements in 1805

  11. JJ Thompson1903 • Atom can be divided into parts. One of which is an electron. • These are negatively charged particles embedded in a positively charged atom. • Raisins embedded in plum pudding

  12. An atom contains a dense positively charged nucleus. The rest of the atom is mostly empty space where the electrons are. Determined this theory after performing the gold-foil experiment. Rutherford 1909

  13. Rutherford’s Gold-foil Experiment • Rutherford directed alpha particles (radioactive source) which are positively charged and smaller than atoms at a thin piece of gold foil. • He expected all the alpha particles to pass through (detected by the fluorescent screen) with just a few being slightly defected.

  14. Rutherford’s Gold-foil Experiment • Results: • Most of the particles did go straight through (atoms are mostly empty space). • A few were slightly deflected. BUT, some were GREATLY deflected. They were strongly repelled by a dense, positive, central core and bounced back

  15. Bohr 1913 • Electrons are located in specific orbits around the nucleus. • Each electron must contain a certain amount of energy to stay in its orbit. The further the electron is from the nucleus, the more energy it contains. Planetary Model Pg 80-82

  16. Wave – Mechanical Model • Previously matter was considered a particle and energy was considered a wave. • This current model predicts that matter and energy can act like waves or particles – Dual Nature Concept • In this model (aka - the electron cloud model), the electrons are in orbitals, which are defined as regions of the most probable electron location. Pg 82-85 (2.9-2.10)

  17. Bohr’s Model versus the Wave – Mechanical Model • The difference is in the description of electron location around the nucleus. • Bohr suggested well defined, fixed orbits. • The wave-mechanical model shows electrons located around the nucleus in orbitals. • An orbital is a region in which an electron with a certain amount of energy is most likely to be located (like a cloud).

  18. Rutherford’s Ghost – 2:30 min • http://www.youtube.com/watch?v=ic5Q3_W7q7w&feature=related • Electron in motion – wave mechanical model – 1 min – notice electrons don’t stay in a single path, more of a vibration cloud • http://www.youtube.com/watch?v=32uEvwxNJvE&feature=related

  19. The Nucleus • Contains both protons and neutrons • Similar in size • Protons are positively charged • Neutrons are not charged, they’re neutral • So overall charge of the nucleus is POSITIVE Pg 70-75 (2.5-2.6)

  20. Atomic Number • Equals the number of protons in an atoms nucleus. • It identifies the element. • It NEVER changes unless the element has changed. • All atoms of Lithium will have 3 Protons.

  21. Nucleus of atom like Nucleus inside of cell • Both contain information that is critical for identification • Cell nucleus contains DNA that identifies the functions of that cell. • Atomic nucleus contains a certain number of protons that identifies the element and its properties.

  22. Mass Number • Equals the number of Protons + Neutrons in the nucleus. • Does NOT identify the element. • Li : mass # = 7 • The # of neutrons an the nucleus can change thus mass # can change.

  23. Isotopes • Atoms of the same protons but with a different number of neutrons. • The number of protons does NOT change.

  24. Isotopes 31H = H31 =H3= H-3

  25. 126C 136C 146C • The Element is __________ • The number 6 refers to the # of ________ • The numbers 12,13,14 refer to the # of _______ • How many protons and neutrons are in the first isotope? • How many protons and neutrons are in the second isotope? • How many protons and neutrons are in the third isotope?

  26. Atomic mass • Decimal • Average of all the isotopes that occur in nature. C-12 C-13 C-14

  27. Calculating Atomic Mass • Of all the naturally occurring Copper, 30.8% are atoms of Copper-65 and 69.2% of copper-63. What is the atomic mass of Cu? • Step 1 - convert percentages into decimals 30.8/100 = .308 69.2/100 = .692

  28. Step 2 – Calculate the contribution of each isotope to the atomic mass by multiplying the decimal percentage by the mass # for each isotope. 0.308 x 65 AMU = 20.2 AMU 0.692 x 63 AMU = 43.596 AMU • Step 3 – Add them together to get the weighted average for the atomic mass. 20.2 AMU + 43.596 AMU 63.796 AMU

  29. Uranium Calculate ATOMIC MASS

  30. Boron Calculate ATOMIC MASS

  31. Discovering the elements • Handout is Introduction to the elements • 36 min from intro to size of atoms segment • http://player.discoveryeducation.com/index.cfm?guidAssetId=2113C4B6-CECB-42E5-B8E4-1244EB5EC32F&blnFromSearch=1 • Physical Science Series: Atomic Structure and the Periodic Table • 11 min from intro thru electron segment • Handout is atomic structure • http://player.discoveryeducation.com/index.cfm?guidAssetId=298799C9-686A-461A-A060-851A721FB678&blnFromSearch=1

  32. Electrons 101 • Found in energy levels around the nucleus (orbitals according to the wave-mechanical model) • Negatively charged • Very, Very, Very small • When atoms are neutral (no charge), protons = electrons, Na0. • Can be gained or lost from the outer most energy level • Valence electrons are found in the valence shell. • These are responsible for most chemical reactions and in the formation of compounds. • Every atom wants 8 valence electrons (unless it has only 1 energy level, then it wants only 2).

  33. Valence Electrons In general, the number of valence electrons affects the chemical properties of an element. Valence electron # = Group # of the periodic table.

  34. unless it has only 1 energy level, then it wants only 2

  35. In an effort to achieve an octet atoms becomes charged and IONS are formed.

  36. Ion Types - Cations • Sodium has 3 orbits (Bohr Model) • The third orbit has 1 electron. • To be more stable • give away the only electron it has in the third orbit • receive 7 more electrons from another atom in order for it to have 8 electrons on the outer orbit. • Both processes would have sodium ending up with 8 electrons on its outer orbit. • Giving away 1 electron is easier than receiving 7 electrons. • Sodium will lose 1 electron which means that it now has 10 electrons and 11 protons. • It has 1 less electron than proton so it’s charge is +1. • Na --> Na+1 + 1e Cats are +

  37. Ion Types - Anions • Oxygen has 2 orbits (Bohr Model). • The second orbit has 6 electrons. • To be more stable • give away all the 6 electrons on the second orbit • receive 2 more electrons from another atom. • Both processes will lead to oxygen having 8 electrons on its outer orbit. • receiving 2 more electrons from another atoms is easier than giving away all its 6 electrons. • Oxygen will receive 2 more electrons which means it now has 10 electrons and 8 protons. • It has 2 more electrons than protons so it’s charge is -2. • O + 2e --> O-2 + 2 e

  38. IONS

  39. Oxidation Number Ionic Charge = Oxidation Number

  40. Na and Cl

  41. Ca and Cl

  42. Al and O

  43. Counting Subatomic Particles • Bi • Number of protons = a • Number of electrons = b • Number of neutrons = c • Atomic number = 83 • Mass # = 209 • As-3 • Number of protons = 33 • Number of electrons = a • Number of neutrons = 42 • Atomic number = b • Mass # = c Atomic Mass = Mass #

  44. Counting Subatomic Particles • Os+4 • Number of protons = a • Number of electrons = b • Number of neutrons = 114 • Atomic number = 76 • Mass # = c • Te+6 • Number of protons = 52 • Number of electrons = a • Number of neutrons = b • Atomic number = c • Mass # = 128 Atomic Mass = Mass #

  45. http://player.discoveryeducation.com/index.cfm?guidAssetId=AE2C7A14-611A-4857-86F2-66933E4C286A&blnFromSearch=1&productcode=UShttp://player.discoveryeducation.com/index.cfm?guidAssetId=AE2C7A14-611A-4857-86F2-66933E4C286A&blnFromSearch=1&productcode=US • How boron ions form – 2 min

  46. Lewis Dot Diagrams • Show only Valence Electrons for the element. • Steps for drawing them • Write the elemental symbols for the atoms • Fill in the electrons • If more than 2, place 1 electrons at each side of the element symbol and then double up as needed. • If there are 2 valence electrons, place both of them on the same side of the element symbol. S Ca

  47. Atoms versus Ions O vs O-2 Mg vs Mg+2 P vs P-3

  48. Lewis Dot Diagrams • Cations have NO electrons in the outermost orbital. • Anions have 8 in the outermost orbital. +1 Cs -1 I

  49. +2 +1 Zn Ag Which diagrams show a full valence shell?

  50. Electrons 102 • Each electron in an atom has its own distinct amount of energy. • depending on their orbital • Electrons in orbitals closer to the nucleus have less energy and are more stable • Electrons in orbitals further from the nucleus have more energy and are less stable • When all electrons in an atom are in their lowest possible energy level, the atom is at its ground state. • The number of electrons found in each orbital when an atom is at the ground state can be found on the periodic table. • This is the atoms electron configuration. Pg 76-79 (2.7-2.8)

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